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(1.4/Atomic Mass of carbon) X Avogadro's number = 1.4/12.0 X 6.02 X 1023 = 7.0 X 1022 atoms, to the justified number of significant digits.
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∙ 14y ago
To determine the number of atoms in 1.4 g of carbon, you first need to convert grams to moles by using the molar mass of carbon (12.01 g/mol). Then you can use Avogadro's number (6.022 x 10^23 atoms/mol) to calculate the number of atoms in one mole of carbon. Finally, multiply the number of moles by Avogadro's number to find the number of atoms in 1.4 g of carbon.
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How many atoms of C are in a 56 g?
The number of atoms is 28,099.10e23.
How many carbon atom are in 5.60 g of glucose?
5.60 g C6H12O6 (1 mole C6H12O6/180.156 g)(6 moles C/1 mole C6H12O6)(6.022 X 1023/1 mole C) = 1.12 X 1023 atoms of carbon ======================
How many atoms of sulfur (S) are in 5 g of sulfur?
5 g of sulfur contain 0,94.10e23 atoms.
What statement about krypton is not true A its molar mass is 83.798 g per mol Kr B Its atomic number is 36 C one mole of krypton atoms has a mass of 41 point 90g D it is a noble gas?
Statement C is not true. One mole of krypton atoms has a mass of approximately 83.798 g, not 41.90 g.
What is the mass of 5.49E25 nitrogen atoms?
6.02 x 1023 atoms of nitrogen will weigh 14 g.So, 5.49 x 1025 atoms of nitrogen will weigh 1277 g.
How many Atoms are in 169g of c?
169 g C x 1 mole C/12.011 g x 6.02x10^23 atoms/mole = 8.47x10^24 atoms
How many carbon atoms are contained in 85.9 g of carbon?
There are 7.16 moles of carbon in 85.9 g of carbon (85.9 g / 12 g/mol). Since there are 6.022 x 10^23 atoms in 1 mole of carbon, the number of carbon atoms in 85.9 g is 4.31 x 10^24 atoms.
How many atoms of C are in a 56 g?
The number of atoms is 28,099.10e23.
How many atoms are in a 12 g of C?
To find the number of carbon atoms in 12 g of carbon (C), you first need to calculate the number of moles of carbon (C) in 12 g using its molar mass. Then, you can use Avogadro's number (6.022 x 10^23) to determine the number of atoms in that many moles of carbon (C).
What is the ratio of c g and o atoms in cerbohydrates?
The general ratio in carbohydrates is approximately 1 carbon atom to 2 hydrogen atoms to 1 oxygen atom (1:2:1). This ratio varies depending on the specific type of carbohydrate and its structure.
How many atoms are in 1.6 g C?
There are approximately 1.34 x 10^22 carbon atoms in 1.6 g of carbon. This calculation is based on the molar mass of carbon (12 g/mol) and Avogadro's number (6.022 x 10^23 atoms/mol). To find the number of atoms, divide the mass of the sample by the molar mass of carbon, and then multiply by Avogadro's number.
How many atoms of carbon (C) are in 0.08 g of carbon?
To find the number of carbon atoms in 0.08 g of carbon, you need to calculate using Avogadro's number and the molar mass of carbon. The molar mass of carbon is approximately 12 g/mol. First, convert grams to moles by dividing 0.08 g by the molar mass of carbon to get approximately 0.0067 moles of carbon. Then, multiply the number of moles by Avogadro's number (6.022 x 10^23) to find that there are approximately 4 x 10^21 atoms of carbon in 0.08 g.
How many atoms are in 49.1740 g of zirconium?
49.1740 g (6.02 x 1023 atoms) / (91.22 g) = 3.25 x 1023 atoms
How many moles of atoms are contained in 5.21x10E24 C2H2?
To find the number of moles of atoms in a compound, first calculate the molar mass of the compound (12 g/mol for carbon, 1 g/mol for hydrogen). Then divide the given number of atoms by Avogadro's number (6.022 x 10^23 atoms/mol) to find the number of moles. In this case, 5.21x10^24 atoms of C2H2 would be equivalent to approximately 8.65 moles.
How many atoms of carbon c are in 0.09 g of carbon?
There are 0.75 moles of carbon in 0.09 g. Since there is 1 mole of carbon contains 6.022 x 10^23 atoms, there are 4.52 x 10^22 atoms of carbon in 0.09 g.
How many atoms are present in helium lithium beryllium boron carbon nitrogen and oxygen?
Helium has 1 atom, lithium has 1 atom, beryllium has 1 atom, boron has 1 atom, carbon has 1 atom, nitrogen has 1 atom, and oxygen has 1 atom, in their natural state.
How many atoms of carbon are in a pure sample of carbon having a mass of 72.0 g?
There are 6.022 x 10^23 atoms in 1 mole of carbon. The molar mass of carbon is 12 g/mol. Therefore, in 72.0 g of carbon, there are (72.0 g / 12 g/mol) * 6.022 x 10^23 atoms = 3.61 x 10^24 atoms of carbon.
